Redox And Group 2 Flashcards
Define oxidation (4)
Oxygen addition
Hydrogen loss
Electron loss
Increase oxidation number
Define reduction (4)
Oxygen loss
Hydrogen addition
Electron gain
Decrease oxidation number
Oxidation number
Measure of how oxidised an atom is
Oxidation number rules (9)
Simple ion = charge
Atom as pure element = 0
F = always -1
O = -2 (except F compounds)
Cl = -1 (except O/F compounds)
H = 1+ (except metal hydrides)
Group 1 = always 1+
Group 2 = always 2+
Al = always 3+
Sum of oxidation number rule (3)
Must be equal on both sides
Sum of ONs in a compound = overall charge
Quoted per atom not compound
Balancing redox equations using ONs
Identify atoms being O/R
Balance amount each is being O/R by
Don’t change O/R ratio
Total left/right charges, balance
Half equation electron placement
O = right
R = left
Half equations (5)
R or O
Feature electrons
2X —> ionic equ
Reversible (depends on other elements reactivity)
Ionic equations (4)
1 O, 1 R
Balance e no
Cancel common terms
H+ and OH- on same side —> H2O
Disproprotionation
Element in a species O and R simultaneously
Eg. 2Cu+ —> Cu + Cu2+
Ionic radius group 2 strand
Smaller up the group
Less electron shells
Less shielding
Electrons held tighter
Electrostatic attraction is stronger despite constant charge
Ionisation energy group 2 trend
Decreases down the group
More electrons, more electron shells
More shielding from positive nucelus
Outer electrons further from nucleus
Reduces attraction despite nuclear charge being constant
Easier to remove electrons
Reactivity trend group 2
Increases down the group
React by losing outer electrons —> Mg2+
Higher IEs, harder to do
Lower IEs = more reactive
Group 2 reaction with water trends
Make metal hydroxides and hydrogen
Be - doesnt react
Mg - very slowly reacts, ppte
Ca - steadily, ppte
Sr - fairly quick, clear solution
Ba - rapid, clear solution
Magnesium reaction with steam
Forms MgO rapidly
Bright white light
Hydrogen gas as it leaves tube (safety)